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Biol 1406 Exam 1
Chapters 1-4
| Term | Definition |
|---|---|
| The 7 characteristics of life | Order Response to stimuli Growth and development Reproduction Evolution and adaptation Regulation Energy processing |
| Levels of organization | atoms -> molecules -> organelles -> cells -> tissues -> organs -> organ systems -> organism -> population -> community -> ecosystem -> biosphere |
| Concept of evolution by natural selection | Organisms with traits that suit their environment are more likely to survive long enough to pass on their advantageous traits to their offspring |
| Inductive reasoning | Specific applied to situations in general |
| Deductive reasoning | General observations applied to specific situation |
| Two groups in controlled experiments | Control group (kept unchanged) Experimental group (changed with independent variable) |
| Cohesion | A molecule’s ability to stick to itself |
| Adhesion | A molecule’s ability to stick to something else |
| Surface tension | How much force it takes to break the surface of a liquid |
| Specific heat | How much it takes to raise the temp of one gram of a substance by 1 degree C |
| The four emergent properties of water | Cohesion Adhesion Surface tension Specific heat |
| Ex of adhesion | Water molecules sticking to the roots to pull themselves up |
| Ex of cohesion | Water droplets sticking together after spilling on the table |
| Ex of surface tension | A glass of water not spilling after being filled over the top |
| Kinetic energy | The energy of motion |
| Water’s special kind of kinetic energy | Thermal energy |
| Water’s specific heat | Being able to absorb large amounts of heat with only a slight change in its own temperature |
| Solution | Mixture where one substance dissolves into another |
| Solvent | Where the substance is dissolved |
| Solute | The substance that is dissolved |
| Water is the universal | Solvent |
| Water is a _ molecule | Polar |
| A singlewater molecule has _ poles of charge | Four |
| Polar molecules have | Poles of partially positive and partially negative charges |
| Non-polar molecules | Have the electrons dispersed equally, and thus are not charged |
| Matter is | Anything that has mass and takes up space |
| An element cannot be | broken down into other substances |
| Trace elements are | required by an organism in small quantities |
| The 4 elements that make up 96% of the world's matter are | Carbon, hydrogen, oxygen, nitrogen |
| Elements are made | of atoms |
| In an uncharged atom, protons and electrons are | equal in number |
| Isotopes | Atoms with differing numbers of neutrons |
| Atomic number | # of protons |
| Mass # | Protons + neutrons |
| Energy level "seats" | 2 -> 8 -> 8 |
| Biosphere | Area of Earth where life exists |
| Genetic sequencing | Basis for modern taxonomy |
| 3 domains | Eukarya Archaea Bacteria |
| The most diverse domain | Eukarya |
| Linnaeus classified organisms by their | physical characteristics |
| Cells illustrate the correlation of | structure and function |
| 2 types of cells | Prokaryote Eukaryote |
| Autotroph | Producers |
| Heterotroph | Consumers |
| Saprophytes | Decomposers |
| Electronegativity | How much an atom is able to attract electrons |
| Electronegativity depends on | # of valence electrons Atomic radius |
| _ valence electrons, electronegativity _ | More; increases |
| Electronegativity difference is greater than 1.7 | bond is ionic |
| Electronegativity is between 1.7 and 0.4 | Bond is polar covalent |
| Electronegativity is less than 0.4 | Bond is non-polar covalent |
| Covalent bonds have an electronegativity of | less than 1.7 |
| Bonding capacity/valency | how many electrons an atom has available for bonding |
| Valence electrons determine the _ of an atom | chemical behavior |
| Ionization | When an atom gains or loses electrons |
| Periods | rows |
| Groups | columns |
| _ increases down the groups | # of electron shells |
| Across the periods | # of valence electrons inc |
| Carbon atomic # | 6 |
| Hydrogen atomic # | 1 |
| Oxygen atomic # | 8 |
| Nitrogen atomic # | 7 |
| Types of chemical bonds | Ionic Covalent Hydrogen |
| Single covalent bonds | One pair of electrons shared (2 total) |
| Double covalent bonds | Two pairs of electrons shared (4 total) |
| Triple covalent bonds | 3 pairs of electrons shared (6 total) |
| Heat of vaporization | heat a liquid must absorb for 1 g to be converted to gas |
| Evaporative cooling | When the water molecules with the highest thermal energy escape as gas, leaving the cooler molecules behind |
| Ex of evaporative cooling | Sweat |
| Water _ upon freezing, allowing ice to _ | expands and is less dense; float |
| Four emergent properties of water | Cohesive behavior Ability to moderate temperature (Specific heat) Expansion upon freezing Versatility as a solvent |
| Acid inc | the [H+] of a solution, between 0-6 on pH scale |
| Base dec | the [H+] of a solution, between 8-14 on pH scale |
| Each pH units represents a _ change in the _ | tenfold (x 10); concentration of [H+] |
| Concentrations are measured in | moles (M or M/l) |
| [H+] and [OH-] must add up to | 14 |
| [H+] = | 1x10^-pH |
| pH = | log exponent of [H+] |
| Buffer | Substance that can minimize changes in pH |
| Buffers do their job by | Absorbing [H+] when in excess or donating it when it's depleted |
| pH of human blood is about | 7.4 |
| Buffers are usually a mix of a | weak acid and its related base |
| Life's molecular diversity is based on the properties of | carbon |
| 4 major classes of organic molecules | Carbohydrates Lipids Proteins Amino acids |
| Inorganic molecules don't | have Carbon-Hydrogen bonds |
| Carbon-based molecules are called | Organic compounds |
| Carbon can form infinite chains of | complex molecules |
| Bonding capacity of carbon | 4, bonds especially well with other carbons and hydrogen |
| Carbon skeleton | chain of carbon atoms |
| Isomers | Compounds with the same molecular formula but different structural arrangements and properties |
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